EP1494967A1 - Verfahren und kit zur herstellung von chlordioxid im gemisch mit sauerstoff - Google Patents
Verfahren und kit zur herstellung von chlordioxid im gemisch mit sauerstoffInfo
- Publication number
- EP1494967A1 EP1494967A1 EP02795029A EP02795029A EP1494967A1 EP 1494967 A1 EP1494967 A1 EP 1494967A1 EP 02795029 A EP02795029 A EP 02795029A EP 02795029 A EP02795029 A EP 02795029A EP 1494967 A1 EP1494967 A1 EP 1494967A1
- Authority
- EP
- European Patent Office
- Prior art keywords
- chlorite
- solutions
- solution
- peroxomonosulfate
- chlorine dioxide
- Prior art date
- Legal status (The legal status is an assumption and is not a legal conclusion. Google has not performed a legal analysis and makes no representation as to the accuracy of the status listed.)
- Granted
Links
Classifications
-
- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
- C01B11/00—Oxides or oxyacids of halogens; Salts thereof
- C01B11/02—Oxides of chlorine
- C01B11/022—Chlorine dioxide (ClO2)
- C01B11/023—Preparation from chlorites or chlorates
- C01B11/024—Preparation from chlorites or chlorates from chlorites
Definitions
- the invention relates to a method for producing chlorine dioxide and a kit for producing chlorine dioxide from ready-to-use reagents.
- Chlorine dioxide is the technically most important chlorine oxide and is mainly used for bleaching, disinfecting and deodorising, but it is difficult to handle, since the gaseous CI0 2 easily escapes from solutions and is explosive from a partial vapor pressure of 100 mbar (20 ° C).
- DE 195 29 504 A1 already discloses a process for the preparation of aqueous chlorine dioxide solutions by oxidation of chlorite with oxo acids and / or oxo acid anions of suitable redox potential in a buffered aqueous medium.
- An oxo-acid solution with a pH value of 5 or less is mixed with an aqueous chlorite solution in a pH-buffered system.
- Phosphate buffers that are very problematic from an environmental point of view are preferably used for buffering.
- the described use of phosphoric acid as a pH regulator takes place in a concentration of approx. 8 g H 3 P0 4 / l, which is too much according to current ideas.
- the process is to be carried out in stirred tanks or flow tubes, the starting materials sodium hypochlorite and phosphoric acid being only available in liquid form.
- the method is therefore unsuitable for use on a small scale with means that are easy to handle.
- the chlorine dioxide solution produced with the method according to the examples is hypochlorite-containing, which is the advantage of Chlorine dioxide destroys.
- the process has the serious disadvantage that chlorates form in the stated procedure and under the specified conditions, for example when hypochlorite solution is combined with phosphoric acid. As described by D'Ans, J. and Freund, HEZ, Elektrochem. Ber. Bunsenges. physics.
- hypochlorous / hypochlorite starting solutions acidified with phosphoric acid and the hypochlorous acid / hypochlorite-containing chlorine dioxide preparation contain chlorate, which should however be avoided.
- peroxomonosulfate - as mentioned alternatively - chlorates are formed as described in the literature:
- DE 195 18 464 describes moldings for the production of chlorine dioxide by subsequent reactions in which chloride is first oxidized to chlorine by means of peroxomonosulphate and further chlorite to chlorine dioxide by the chlorine formed.
- DE 195 184 64 uses compatible basic additives such as sodium hydrogen carbonate, sodium carbonate decahydrate and disodium hydrogen phosphate dodecahydrate (see column 2, lines 18, 19).
- the indication of the acidic component "metal hydrogen sulfate" with a 15% content is based on the fact that the percentage of potassium hydrogen sulfate in the caroate has been converted. This means that no sodium hydrogen sulfate has been added.
- the basic constituents mentioned above stoichiometrically neutralize the potassium hydrogen sulfate of the caroate, so that the pH of the reaction solution is approximately in the neutral range.
- the initial concentration ratio of chlorite to chlorous acid would be 100,000: 1.
- peroxomonosulfuric acid is only stable in the acidic range and otherwise disproportionates to sulfuric acid and oxygen, the pH should therefore remain in the acidic range for the peroxomonosulfuric acid components throughout the process, but especially at the beginning of the process.
- the invention has for its object to provide a simple and safe to use method with which chlorine dioxide can be freshly produced if necessary.
- the reaction should take place with a short reaction time at low temperature, i.e. not necessarily significantly above room temperature.
- the formation of chlorine and chlorates should be avoided.
- the process should also be manageable on a small scale using simple means, for example to be suitable for private swimming pools or for small-scale drinking water disinfection.
- the object is achieved by means of a process for the production of chlorine dioxide in a mixture with oxygen by reaction of chlorite with peroxomonosulfate in the presence of a redox initiator in an acidic aqueous solution. Further refinements of the method are characterized in the subclaims.
- kits for producing chlorine dioxide in a mixture with oxygen are provided to achieve the object, in particular for water treatment, which has ready-to-use solutions and / or dry compositions, a ready-to-use solution or dry composition containing at least one chlorite and a second ready-to-use solution or dry composition contains at least one peroxomonosulfate in a mixture with a redox initiator, such as preferably peroxodisulfate and / or oxalic acid.
- a redox initiator such as preferably peroxodisulfate and / or oxalic acid.
- the invention thus provides a method with which chlorine dioxide can be produced practically quantitatively after a reaction time of less than 30 minutes in acidic aqueous solution at a temperature already below room temperature (from 10 ° C. in under 30 minutes).
- the method uses the reaction of chlorite with peroxomonosulfate (also called carat, salt of Caro's acid) according to the following reaction equation
- the resulting radicals, the sulfate radical anion, the peroxomonosulfate radical anion and the carboxyl radical accelerate the formation of chlorine dioxide. At the end of the reaction, they are completely converted to sulfate or hydrogen sulfate and carbon dioxide.
- the process takes place without hydrogen sulfate and also without chloride in satisfactory yields, but both the use of chloride and hydrogen sulfate is preferred.
- the use of the catalysts (H + and CI) is particularly advantageous if the reaction is to be carried out at room temperature.
- chloride accelerates the catalytic decomposition of the intermediate hydrogen peroxide with the formation of singlet oxygen 1 0 2 and water and prevents the formation of chlorates.
- alkali halides have proven to be particularly advantageous since they catalyze the decomposition of hydrogen peroxide.
- the intermediate hydrogen peroxide decomposes into oxygen and water and can no longer react with the main reaction product chlorine dioxide, which leads to a quantitative conversion and to a constant concentration of chlorine dioxide.
- the addition of hydrogen sulfate exponentially increases the oxidation effect of peroxomonosulfate, since the individual potential of the redox couple increases according to Nemst's equation:
- chlorine dioxide is therefore prepared in a mixture with oxygen by reacting chlorite with peroxomonosulfate (educts) in acidic aqueous solution in the presence of a redox initiator, it being possible to add hydrogen sulfate and / or chloride.
- Sodium chlorite is preferably used as the chlorite, but other chlorites or mixtures thereof can optionally be used.
- Potassium peroxomonosulfate is preferably used as the peroxomonosulfate.
- a potassium peroxomonosulphate triple salt (Degussa) commonly used under the name Caroat can be used.
- Hydrogen sulfate and chloride preferably sodium hydrogen sulfate and sodium chloride, are used as additives with a catalytic property.
- the procedure should be carried out at a pH between 1.5 and 3.5.
- the pH is preferably adjusted using the hydrogen sulfate
- the process can be carried out at any temperature between room temperature and the boiling point of the water, an increase in the temperature leading to shorter reaction times, but the resulting CI0 2 can also escape more easily from the heated solution.
- the process is preferably carried out at temperatures from 10 ° C., at room temperature or around 30 to 45 ° C.
- the heating can take place either before the start of the reaction (heating of the starting material solutions) or during the reaction (after adding the unheated starting material solutions). If the reagents are dissolved in warm water and no further heat is added in the course of the reaction, the initial water temperature may rise advantageously be about 75 to 95 ° C. It is particularly preferred to carry out the process at unchanged water temperature of the water to be treated, if this is 10 to 50 ° C.
- the process described here works according to the invention in an acidic environment, the pH preferably being about 2 in order to increase both the oxidation effect of peroxomonosulfate (see Eq. III) and to increase the concentration of chlorous acid.
- the chlorous acid is easier to oxidize to chlorine dioxide than its conjugate base (chlorite).
- chlorite conjugate base
- the competitive reaction - chlorine formation - can be largely eliminated, as the kinetic measurements show that no chlorine can be determined.
- the pH can only be increased after the reaction has ended by adding bases (see Example 5).
- a stabilizer system for stabilizing the pH between about 3.5 and 6.8 is added in a further development of the invention. This is preferably at least one of the following substances:
- Borate in particular perborate, fluoride, percarbonate, basic magnesium carbonate or a mixture of at least two of these substances.
- the method according to the invention has numerous advantages over the methods known in the prior art.
- the simultaneous generation of oxygen (equation I) dilutes the chlorine dioxide formed without impairing its effect.
- the process produces neither chlorine nor chlorates, and there is no chlorine regression (by reducing chlorine dioxide to chlorite).
- the process enables for the first time a practically complete conversion of the educts to chlorine dioxide; with a suitable choice of stoichiometric ratios, neither chlorite nor peroxides are detectable at the end of the reaction.
- a first solution contains a chlorite, preferably sodium chlorite, and a chloride, preferably sodium chloride.
- a second solution contains a peroxomonosulfate (carat), preferably potassium peroxomonosulfate, the redox initiator, as described above, and optionally a hydrogen sulfate, with which the desired pH is adjusted more precisely between 1.5 and 3.5 and in any case below 5 can be, preferably sodium bisulfate.
- the solutions are then combined, mixed and, if necessary, heated.
- the combined solutions can be heated, or the individual solutions provided can be heated or prepared with warm or hot water and then combined.
- the combined solutions can be shaken or stirred for better mixing.
- Gaseous chlorine dioxide is explosive from a concentration of 300 mg / l or 10 vol.%.
- the escaped oxygen dilutes the gaseous chlorine dioxide so that it is less dangerous, especially in closed systems, e.g. Reactors, storage containers, is to be handled.
- This method produces approx. 10 times the amount of oxygen than the solubility of oxygen in water (approx. 0.04 g / l).
- the gas phase (above the chlorine dioxide solution in the closed system) consists of approx. 20% oxygen and 80% chlorine dioxide.
- Chlorite, chloride, caroate, hydrogen sulfate and peroxodisulfate are mixed in water give and the solution is heated.
- the reagents can also be added to warm to hot water and then only mixed or shaken.
- Chlorite and chloride are dissolved in water in a first solution, caroate and hydrogen sulfate are dissolved in water in a second solution, the two solutions are combined and heated. In addition, a peroxodisulfate is added to the second solution.
- Chlorite and chloride are dissolved in water, caroate, peroxodisulfate or oxalic acid and hydrogen sulfate are pressed together dry, the pressing or the tablet is added to the solution, which is heated and stirred if necessary.
- the invention further comprises kits in which the method can be carried out with the aid of ready-to-use solutions.
- the kit according to the invention for producing chlorine dioxide mixed with oxygen comprises ready-to-use solutions and / or dry compositions, a ready-to-use solution or dry composition containing at least one chlorite and a second ready-to-use solution or dry composition containing at least one peroxomonosulfate and one peroxodisulfate or oxalic acid.
- the chlorite-containing solution or dry composition may additionally contain chloride and the other hydrogen sulfate.
- the solution or dry composition containing peroxomonosulfate can additionally contain peroxodisulfate and / or hydrogen sulfate.
- the pH value of the ready-to-use solutions is preferably between 9 and 12.5 for the reducing chlorite-containing solution and between 1.7 and 3.5 for the oxidizing peroxomonosulfate-containing solution.
- the molar ratio of the corresponding acid-base pair (HS0 4 7S0 4 2 " ) of the oxidizing solution is preferably 1-3.
- the pH of the reducing chlorite solution is preferably 11.
- the pH is preferably adjusted using hydroxides or carbonates Alkali or Alkaline earths.
- the pH of the finished chlorine dioxide solution can preferably be increased to pH 5.0-6.5 by adding preparations of alkali metal carbonates, alkaline earth metal carbonates or alkali metal phosphates in liquid form, powder or tablet form.
- the ready-to-use solutions are available in suitable containers and, if necessary, are mixed in a mixing container to carry out the process.
- One of the solution containers into which the other solution is added can be provided as the mixing container.
- the volumes of the containers must be selected accordingly.
- the kits can also be used very well in plants for the continuous or periodic production of chlorine dioxide. This is possible without any special adjustments to the systems.
- Dry preparations can also be used, so that the kit either contains at least two dry preparations which are dissolved in water together for the implementation of the method, or a dry preparation and a ready-to-use solution. It is currently preferred to use a solution of sodium chlorite and sodium chloride in water in conjunction with a pressing of caroate and potassium hydrogen sulfate.
- the dry preparations can be in the form of pellets or tablets or in the form of granules or powder packed in portions.
Landscapes
- Life Sciences & Earth Sciences (AREA)
- General Life Sciences & Earth Sciences (AREA)
- Geology (AREA)
- Chemical & Material Sciences (AREA)
- Organic Chemistry (AREA)
- Inorganic Chemistry (AREA)
- Agricultural Chemicals And Associated Chemicals (AREA)
- Food Preservation Except Freezing, Refrigeration, And Drying (AREA)
- Organic Low-Molecular-Weight Compounds And Preparation Thereof (AREA)
- Catalysts (AREA)
Description
Claims
Applications Claiming Priority (3)
Application Number | Priority Date | Filing Date | Title |
---|---|---|---|
DE10164106 | 2001-12-24 | ||
DE10164106A DE10164106A1 (de) | 2001-12-24 | 2001-12-24 | Verfahren und Kit zur Herstellung von Chlordioxid im Gemisch mit Sauerstoff |
PCT/DE2002/004707 WO2003055797A1 (de) | 2001-12-24 | 2002-12-20 | Verfahren und kit zur herstellung von chlordioxid im gemisch mit sauerstoff |
Publications (3)
Publication Number | Publication Date |
---|---|
EP1494967A1 true EP1494967A1 (de) | 2005-01-12 |
EP1494967B1 EP1494967B1 (de) | 2006-11-15 |
EP1494967B2 EP1494967B2 (de) | 2015-04-15 |
Family
ID=7710960
Family Applications (1)
Application Number | Title | Priority Date | Filing Date |
---|---|---|---|
EP02795029.4A Expired - Lifetime EP1494967B2 (de) | 2001-12-24 | 2002-12-20 | Verfahren und kit zur herstellung von chlordioxid im gemisch mit sauerstoff |
Country Status (6)
Country | Link |
---|---|
EP (1) | EP1494967B2 (de) |
AT (1) | ATE345313T1 (de) |
AU (1) | AU2002360918A1 (de) |
DE (3) | DE10164106A1 (de) |
ES (1) | ES2275019T5 (de) |
WO (1) | WO2003055797A1 (de) |
Cited By (1)
Publication number | Priority date | Publication date | Assignee | Title |
---|---|---|---|---|
US9827542B2 (en) | 2012-05-04 | 2017-11-28 | Fritz Küke | Device and method for producing aqueous chlorine dioxide solutions, and storage units and kits for corresponding usage |
Families Citing this family (12)
Publication number | Priority date | Publication date | Assignee | Title |
---|---|---|---|---|
US7695692B2 (en) | 2003-08-06 | 2010-04-13 | Sanderson William D | Apparatus and method for producing chlorine dioxide |
US20060016765A1 (en) * | 2004-07-21 | 2006-01-26 | Dipietro David G | Water treatment |
DE102005038320B4 (de) * | 2004-08-12 | 2014-01-16 | Helrik Bobke | Transportables Behältnis zur Herstellung eines gasförmigen Desinfektionsmittels |
US7303737B2 (en) * | 2005-11-21 | 2007-12-04 | Gojo Industries, Inc. | Generation of chlorine dioxide |
US7666384B2 (en) | 2008-01-17 | 2010-02-23 | Sanderson William D | Stable chlorine dioxide tablet |
WO2011086579A1 (en) * | 2010-01-18 | 2011-07-21 | Prophylaxis | Process for producing stable and pure liquid form of chlorine dioxide |
DE102013010950B4 (de) | 2012-06-28 | 2016-09-01 | Hochschule Anhalt | Elektrolysezelle und Verfahren zur elektrolytischen Erzeugung von Chlordioxid |
BE1021008B1 (nl) * | 2014-03-12 | 2015-10-13 | Aqua Ecologic | Stabiele chloordioxidesamenstelling en bereidingswijze |
WO2015136478A1 (en) * | 2014-03-12 | 2015-09-17 | Aqua Ecologic | Stable chlorine dioxide composition and method of preparation |
DE102014014188A1 (de) | 2014-09-24 | 2016-03-24 | Hochschule Anhalt (Fh) | Verfahren zur chemischen Erzeugung von Chlordioxid aus Chloritionen und Ozon |
US10400198B2 (en) | 2016-08-25 | 2019-09-03 | Eagle Us 2 Llc | Method of sanitizing a surface |
RU2746551C1 (ru) | 2020-08-31 | 2021-04-15 | Общество с ограниченной ответственностью "АполлО" | Способ получения стабилизированного водного раствора диоксида хлора |
Family Cites Families (8)
Publication number | Priority date | Publication date | Assignee | Title |
---|---|---|---|---|
DE3427119A1 (de) † | 1984-07-23 | 1986-01-23 | Peroxid-Chemie GmbH, 8023 Höllriegelskreuth | Verfahren zur herstellung von kaliumpermonosulfat-tripelsalz |
US5324447A (en) † | 1989-10-02 | 1994-06-28 | Allergan, Inc. | Method and activator compositions to disinfect lenses |
EP0481269B1 (de) † | 1990-10-16 | 1996-12-04 | Hoelzle & Chelius GmbH | Perborat- oder boratfreies Wasseraufbereitungs- und/oder Wasserdesinfektionsmittel, Verfahren zu dessen Herstellung und Verwendung |
DE4117487A1 (de) † | 1991-05-28 | 1992-12-03 | Wacker Chemie Gmbh | Aminooxy-vernetzer enthaltende waessrige dispersionen von carbonylgruppen enthaltenden copolymerisaten |
DE19503900C1 (de) † | 1995-02-07 | 1995-11-23 | Degussa | Verfahren zur Herstellung des Kaliumperoxomonosulfat-Tripelsalzes 2 KHSO¶5¶ . KHSO¶4¶ . K¶2¶SO¶4¶ |
DE19514612A1 (de) | 1995-04-25 | 1996-10-31 | Fritz Dr Kueke | Verfahren zur Herstellung einer wässrigen Chlordioxid-Lösung |
DE19518464C2 (de) * | 1995-05-19 | 1999-01-14 | Khalaf Baerbel | Formling zur Herstellung einer stabilisierten Chlordioxidlösung |
DE19529504C2 (de) * | 1995-08-10 | 1998-03-26 | Manfred Prof Dr Rer Na Rimpler | Verfahren zur Herstellung wäßriger Chlordioxid-Lösungen |
-
2001
- 2001-12-24 DE DE10164106A patent/DE10164106A1/de not_active Withdrawn
-
2002
- 2002-12-20 AU AU2002360918A patent/AU2002360918A1/en not_active Abandoned
- 2002-12-20 WO PCT/DE2002/004707 patent/WO2003055797A1/de active IP Right Grant
- 2002-12-20 DE DE20280429U patent/DE20280429U1/de not_active Expired - Lifetime
- 2002-12-20 ES ES02795029.4T patent/ES2275019T5/es not_active Expired - Lifetime
- 2002-12-20 AT AT02795029T patent/ATE345313T1/de not_active IP Right Cessation
- 2002-12-20 EP EP02795029.4A patent/EP1494967B2/de not_active Expired - Lifetime
- 2002-12-20 DE DE50208737T patent/DE50208737D1/de not_active Expired - Lifetime
Non-Patent Citations (1)
Title |
---|
See references of WO03055797A1 * |
Cited By (1)
Publication number | Priority date | Publication date | Assignee | Title |
---|---|---|---|---|
US9827542B2 (en) | 2012-05-04 | 2017-11-28 | Fritz Küke | Device and method for producing aqueous chlorine dioxide solutions, and storage units and kits for corresponding usage |
Also Published As
Publication number | Publication date |
---|---|
ES2275019T5 (es) | 2015-07-16 |
DE50208737D1 (de) | 2006-12-28 |
WO2003055797A1 (de) | 2003-07-10 |
EP1494967B2 (de) | 2015-04-15 |
ATE345313T1 (de) | 2006-12-15 |
EP1494967B1 (de) | 2006-11-15 |
DE10164106A1 (de) | 2003-07-10 |
ES2275019T3 (es) | 2007-06-01 |
AU2002360918A1 (en) | 2003-07-15 |
DE20280429U1 (de) | 2005-04-07 |
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